Octane (C3H18) undergoes combustion according to the following thermochemical equation:2C3H18(1) + 2502(g)16CO2(g) + 18H20(1)°pxn = -11,020 kJ/mol.Given that AH°{CO2(g)] = -393.5 kJ/mol and AH°{{H2O(1)] = -285.8 kJ/mol, calculate the standard enthalpy of formation of octane.O -420 kJ/molO 22,040 kJ/molO - 210 kJ/molO 420 kJ/molO -11,230 kJ/mol

Given chemical reaction : 2C8H18 + 25 O2 ---> 16 CO2 + 18 H2O

C3H18(1) + 2502(g) - 16CO2(9) + 18H20(1) AH°n = -11,020 KJ/mol. iven that AH°{CO2(9)] = -393.5 kJ/mol and AH?{H2O(1)] = -285.8 kJ/mol, calculate the standard enthalpy of formatio O -420 kJ/mol O 22,040 kJ/mol O -210 kJ/mol O 420 kJ/mol O -11,230 kJ/mol

C3H18(1) + 2502(g) - 16CO2(9) + 18H20(1) AH°n = -11,020 KJ/mol. iven that AH°{CO2(9)] = -393.5 kJ/mol and AH?{H2O(1)] = -285.8 kJ/mol, calculate the standard enthalpy of formatio O -420 kJ/mol O 22,040 kJ/mol O -210 kJ/mol O 420 kJ/mol O -11,230 kJ/mol

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Given the information below: 2C(s) + 2H20(g) CH4(g) + CO2(g) AH° = 35.3 kJ 2C(s) + 2H20(g) 2C0(g) + 2H2(g) AH° = 462.6 kJ -> CH4(g) + H20(g)→ CO(g) + 3H2(g) AH° = -61.2 kJ %3D Calculate the enthalpy of reaction for the reaction below (in kJ) Co(g) + H20(g) → CO2(g) + H2(g) -366,1 kJ -488.5kJ -436.7 kJ +488.5 kJ +436,7 kJ +366.1kJ O0 0 O OO
Question 4 of 17 Using the equations SrO (s) + CO₂ (g) → SrCO3 (s) AH° = -234 kJ/mol 2 Sr(s) + O₂(g) → 2 SrO (s) AH° = -1184 kJ/mol CO₂ (g) → C(s) + O₂ (g) AH° = 394 kJ/mol Determine the molar enthalpy (in kJ/mol) for the reaction 1 4 7 +/- 2 SrCO3 (s) → 2 Sr (s) + 2 C(s) + 3 O₂ (g). 2 5 8 Submit kJ/mol 3 60 9 O Tap here or pull up for additional resources XU x 100
powo 72 3. Calculate the heat of combustion (kJ) of propane, C3H8 using the listed standard enthalpy of reaction data: C3H8(g) + 5 O2(g) →3 CO2(g) + 4 H₂O(g) AH° = -103.8 kJ AH = -393.5 kJ AHO = -241.8 kJ 3 C(s) + 4 H₂(g) →→ C3H8(g) C(s) + O2(g) → CO2(g) H₂(g) + 1/2 O2(g) → H₂O(g) 4. Given the following equations and Ho values given below, determine the heat of reaction at 298 K for the reaction: 2 N₂(g) + 5 O₂(g) →2 N₂O5(g) AHO=-571.6 kJ AH°= -73.7 kJ AH°=-348.2 kJ (24 2 H₂(g) + O2(g) → 2 H₂O(1) N₂Os(g) + H₂O(1)→ 2 HNO3(1) N2(g) + 3 O2(g) + H₂(g) → 2 HNO3(1) HA
b My Questions | bartleby 101 Chem101 app.101edu.co Submit Question 25 of 29 Using the equations N2 (g) + 3 H2 (g) → 2 NH3 (g) AH° = -91.8 kJ/mol C(s) + 2 H2 (g) → H2 (g) + 2 C(s) + N2 (g) → 2 HCN (g) AH° = 270.3 kJ/mol Determine the enthalpy for the reaction CH4 (g) + NH3 (g) → HCN (g) + 3 H2 (g). → CH4 (g) AH° = -74.9 kJ/mol %3D | kJ/mol 1 3 4 8 9. +/- x 100 1:22 PM O Type here to search 12/9/2019 LO
O Macmillan Learning For a particular isomer of Cg H₁g, the combustion reaction produces 5108.7 kJ of heat per mole of Cg H₁ (g) consumed, under standard conditions. 18⁹ 18 C8H₁8 (g) + 25/ 02(g) 8 CO₂(g) + 9 H₂O(g) 2 AH; = ΔΗ AH ixn = -5108.7 kJ/mol What is the standard enthalpy of formation of this isomer of Cg H₁8 (g)? Standard enthalpy of formation values can be found in this table of thermodynamic values. 8 18 kJ/mol
Calculate the enthalpy change for the following reaction, _C₂H4 (9) + using the following standard heats of formation: AH(C₂H4) = +52.5 kJ/mol; AH(CF4) =-933.0 kJ/mol; AH (HF) =-271.6 kJ/mol _F₂(g) → _CF4(g) + _HF(g)
© Macmillan Learning For a particular isomer of Cg H₁8, the combustion reaction produces 5108.7 kJ of heat per mole of Cg H₁8 (g) consumed, under standard conditions. Cg H18 (g) + 25/ 0₂(g) → 8 CO₂(g) + 9 H₂O(g) What is the standard enthalpy of formation of this isomer of Cg H₁g (g)? AH; = esc 1 TOOLS X10" 2 # 3 с $ 4 AHxn=-5108.7 kJ/mol G Search or type URL L 5 MacBook Pro % < 6 & kJ/mol 8
Isooctane (2,2,4-trimethylpentane), one of the many hydrocarbons that make up gasoline, burns in air to give water and carbon dioxide. 2 C3H13 (2) + 25 02 (g) → 16 CO2(g) + 18 H2O(£) A,H° = -10,922 kJ/mol-rxn What is the enthalpy change if you burn 7.50 L of isooctane (d = 0.69 g/mL)? Enthalpy change |kJ =
For a particular isomer of Cg H₁g, the combustion reaction produces 5108.7 kJ of heat per mole of C, H₁g (g) consumed, under standard conditions. 25 Cg H18 (8) + O₂(g) →→→ 8 CO₂(g) + 9 H₂O(g) What is the standard enthalpy of formation of this isomer of Cg H₁g (g)? AH; = $ V T B MacBook Air Y H & 7 8 AH-5108.7 kJ/mol 18 N M K 1 38 kJ/mol
Given the following reactions: N2 (g) + O2 (g) → 2NO (g) AH = +180.7 kJ 2N20 (g) → O2 (g) + 2N2 (g) AH = -163.2 kJ the enthalpy of reaction for 2N20 (g) → 2NOo (g) + N2 (g) is kJ. -343.9 343.9 -145.7 145.7 O 17.5
2 NOCI(g) → 2 NO(g) +Cl2(g) AH° =+75.56 kJ 2 NO(g) + 02(g) → 2 NO2(g) AH° =-113.05 kJ 2 NO2(g) → N2O4(g)AH° =-58.03 kJ Compute AH° of N2O4(g) +Cl2(g) → 2 NOCI(g) + O2(g) in kJ. +246.65 -95.52 -246.65 +95.52 +47.76